Investigation of the Sensing Properties of Lanthanoid Metal–Organic Frameworks (Ln-MOFs) with Terephthalic Acid

The solvothermal synthesis of LnCl3.nH2O with terephthalic acid (benzene-1,4-dicarboxylic acid, H2BDC) produced metal–organic frameworks (LnBDC), [Ln2(BDC)3(H2O)4]∞, where Ln = Sm, Eu, Tb, and Dy. The materials obtained were characterized by a number of physico-chemical techniques. The influence of the ionic radius of the lanthanides on the microstructural characteristics of the Ln-MOFs was evaluated by performing Rietveld refinement. The MOFs obtained were tested as fluorescent sensors for numerous cations and anions in water. The highly luminescent EuBDC and TbBDC demonstrated multi-responsive luminescence sensing functions to detect Ag(I), Fe(III), Cr(III), and Cr(VI), which are essential for their environmental applications. By applying the non-linear Stern–Volmer equation, the fluorescent quenching mechanism was determined. The stability of the obtained materials in water in a wide pH range (acidity pH = 4 and alkalinity pH = 9 solutions) was confirmed.


Introduction
Metal-organic frameworks (MOFs), also known as potential porous coordination polymers, are an emerging class of molecular materials.Due to their structural and functional tenability, investigations based on MOFs are among the fastest-growing scientific fields.These crystalline hybrid materials are built by means of coordination bonds between inorganic metal-containing units and organic ligands.In their construction, secondary building units (the metal-containing nodes) and binding ligands (the organic linkers) can be distinguished [1].This allows modification and control of the pore size, as well as their functionality.The structure obtained can be a one-, two-, or three-dimensional coordination network with potential voids [2].
The lanthanoids Sm, Eu, Tb, and Dy and their trivalent ions possess fluorescence properties in the visible region due to Stokes shift upon activation by near-UV light.Since f→f transitions according to Laporte's selection rules are forbidden, their direct activation is impractical due to the low molar absorption coefficients leading to negligible intrinsic fluorescence [3].This deficiency can be overcome by incorporating the ions into organic and inorganic materials, such as MOFs, which possess groups/ions capable of carrying out charge transfer to the photoactive metal (antenna effect).
Terephthalic acid (benzene-1,4-dicarboxylic acid, H 2 BDC) has been studied as a ligand leading to luminescence enhancement of Ln(III) ions [4].More than 20 different crystal structures of Ln(III) ions synthesized and characterized with terephthalic acid are an illustration of the diversity obtained with a single ligand by varying the synthesis conditions.Both mixed-ligand [5,6] and mixed-metal MOFs [7,8] have been prepared with terephthalic acid.
Among the most common structures obtained with terephthalic acid and Ln(III) is the one presented and discussed in this study, corresponding to the empirical formula [Ln 2 (BDC) 3 (H 2 O) 4 ] ∞ , triclinic, P−1.First, Reineke and co-workers [9] published this structure with Tb(III) and studied its fluorescence properties.Later, Haquin and co-workers studied its NIR luminescence with Er(III) in 2009 [10], and in 2013, their work included five more Ln(III) ions (Tb, Dy, Sm, Eu, and Gd), with a focus on the luminescence color of those materials for potential LED applications [11].In 2009, Daiguebonne et al. reported the synthesis and characterization of coordination polymers with the general formula [Ln 2 (BDC) 3 (H 2 O) 4 ] n , with Ln = Y, La-Lu (except Pm) [12], and expanded the study in 2009 [13] with mixed-metal structures and investigation of their tunable emission.Their polymers also correspond to the structure investigated in this work.Two more reports on the structure in question, one focused on the Ce analogue [14] and the other focused on structural studies involving a comparison with several different structures where the number of coordinated water molecules was not four [15], have been published.In 2013, Cadiau and co-workers suggested materials based on this structure for a radiometric nanothermometer [16].Interestingly, these materials have also been suggested to be used for gunshot residue (GSR) luminescent marking [17].A mechanochemical approach was also reported as a method for their synthesis in 2020 [18].
Investigations on two potential applications of the Ln-MOF mentioned before are scarce in the literature: (i) as catalysts or catalyst carriers in advanced oxidation processes for water and air purification (to be mentioned, our group recently reported some promising results in this field [19]) and (ii) as sensor materials for detecting water pollutants.
Although MOFs are attracting interest as sensor materials [20][21][22][23][24][25][26][27], as far as we are aware, only Zhang and co-workers investigated MOFs with the composition mentioned for detecting picric acid (TNP) [28]; recently, Donghan et al. discussed the fluorescence turn off-turn on continuous response of dual-lanthanide metal-organic frameworks for selectively detecting fluoroquinolone antibiotics [29].So, the focus of this work is on the investigation, in detail, of Ln-MOFs with the composition [Ln 2 (BDC) 3 (H 2 O) 4 ] ∞ (Ln = Sm, Eu, Tb, Dy) as potential sensors for water pollutants.A detailed investigation of the stability of the materials in water, as well as in environments with different acidity levels, and of their activity in different solvents and in the presence of different ions (cations and anions) is included.The latter is rarely discussed in the literature but is important for sensor materials.Structural characteristics play an important role in this type of application; especially, the crystallite size and microstrains play a significant role in the intensity of luminescence, which, in its turn, is essential for sensor application.So, even for isostructural MOFs, these characteristics are essential for sensor performance in a water suspension, and this is the reason information about all samples is extracted by applying Rietveld refinement, which brings novelty to the work, along with all the investigation related to sensor properties.An important aspect of this investigation is the detailed description of non-linear Stern-Volmer data and the possible mechanisms of quenching.

Crystal Structure of DyBDC-Single Crystal (SC)
The experimental details of single-crystal diffraction measurements, as well as corresponding CCDC deposition numbers, are summarized in Table S1 [30].The data can be obtained free of charge from http://www.ccdc.cam.ac.uk/conts/retrieving.html (or from the Cambridge Crystallographic Data Centre, 12, Union Road, Cambridge CB2 1EZ, UK; fax: +44-1223-336033).
Crystals suitable for single-crystal XRD measurements were obtained The crystal packing viewed along the a-axis of DyBDC (DyBDC-SC) is shown in Figure 1.The obtained material was isostructural to the Nd [15], Tb [9], and Er [15] analogues reported earlier and crystallizes in the triclinic P−1 space group.To the best of our knowledge, this is the first report of a Dy analogue structure obtained by single-crystal diffraction.The Dy(III) ions were the center of a distorted DyO 8 (distortion index 0.04243), where the six oxygen atoms belonged to the adjacent terephthalic acid ligand and the other two to the water molecules.The effective coordination number was found to be 7.37, which is due to the fact that the Dy-O distance involving the oxygen atoms of the water molecules is slightly longer, in the range of 2.491(4) Å-2.513(4) Å (average 2.502(4) Å), while the bonds involving the oxygen atoms from the terephthalic acid are in the range of 2.268(3) Å-2.481(4) Å (average 2.340(4) Å).
packing viewed along the a-axis of DyBDC (DyBDC-SC) is shown in Figure 1.The obtained material was isostructural to the Nd [15], Tb [9], and Er [15] analogues reported earlier and crystallizes in the triclinic P−1 space group.To the best of our knowledge, this is the first report of a Dy analogue structure obtained by single-crystal diffraction.The Dy(III) ions were the center of a distorted DyO8 (distortion index 0.04243), where the six oxygen atoms belonged to the adjacent terephthalic acid ligand and the other two to the water molecules.The effective coordination number was found to be 7.37, which is due to the fact that the Dy-O distance involving the oxygen atoms of the water molecules is slightly longer, in the range of 2.491(4) Å-2.513(4) Å (average 2.502(4) Å), while the bonds involving the oxygen atoms from the terephthalic acid are in the range of 2.268(3) Å-2.481(4) Å (average 2.340(4) Å).

Powder X-ray Diffraction
The powder XRD pa erns of all obtained MOFs are presented in Figure 2, which confirms that all the materials were isostructural to each other and to the DyBDC-SC.The phase analysis confirmed that all the XRD peaks belonged to the [Ln2(BDC)3(H2O)4]∞ phase, with no crystalline impurity phases.

Powder X-ray Diffraction
The powder XRD patterns of all obtained MOFs are presented in Figure 2, which confirms that all the materials were isostructural to each other and to the DyBDC-SC.The phase analysis confirmed that all the XRD peaks belonged to the [Ln 2 (BDC) 3 (H 2 O) 4 ] ∞ phase, with no crystalline impurity phases.Insight into the crystal structure and microstructural characteristics of the obtained powders was gained by performing full-profile Rietveld refinement.The results are summarized in Table S2, while the Rietveld refinement profiles are presented in Figure S1.The unit cell volume and unit cell parameters (Figure 2b) of the MOFs slowly decreased from the Sm to the Dy analogue, which is in good agreement with the change in the ionic radius due to lanthanide contraction.Significant differences were observed in the microstructural characteristics of the samples.Despite being prepared by applying the same procedure, a significant difference in the crystallite sizes of the obtained MOFs, with a clear trend of size reduction from Sm to Dy, was observed.In spite of the la er trend mentioned, the microstrain values were virtually the same within the standard deviation.Insight into the crystal structure and microstructural characteristics of the obtained powders was gained by performing full-profile Rietveld refinement.The results are summarized in Table S2, while the Rietveld refinement profiles are presented in Figure S1.The unit cell volume and unit cell parameters (Figure 2b) of the MOFs slowly decreased from the Sm to the Dy analogue, which is in good agreement with the change in the ionic radius due to lanthanide contraction.Significant differences were observed in the microstructural characteristics of the samples.Despite being prepared by applying the same procedure, a significant difference in the crystallite sizes of the obtained MOFs, with a clear trend of size reduction from Sm to Dy, was observed.In spite of the latter trend mentioned, the microstrain values were virtually the same within the standard deviation.

Morphology
The SEM image of the DyBDC-SC (Figure 3a) revealed flat and lamellar crystals with a sheet-like shape and not-so-clearly-defined crystal edges.The SEM images of the polycrystalline samples (Figure 3b-e) showed similar morphological features agglomerated into flower-like pattern lamellae.The particles were polydispersed in size.Despite that, it was noticeable that the smallest average lamellae size was that of the EuBDC, followed by that of the SmBDC, while the TbBDC and the DyBDC were almost identical in size.

Optical Properties
Emissions of the powdered samples with four different Ln(III) ions were recorded (Figure 4a) under the same conditions (λex = 320 nm; ex/em slit 5/1.5 nm; data interval 1.0 nm; average time 0.10 s; PMT voltage 800 V).The most intensive emission was detected for TbBDC, followed by EuBDC.Emission from SmBDC and DyBDC was also present, as can be seen from the normalized spectra (Figure S2), but obviously, terephthalic acid is not a good sensitizer of their luminescence, observed as well in [11].A possible explanation is the small energy gap possessed by Dy(III) and Sm(III) [31], which favors nonradiative deactivation, especially in the presence of coordinated water molecules.The energy of the lowest triplet state of terephthalic acid, 23,530 cm -1 [11], happens to be

Optical Properties
Emissions of the powdered samples with four different Ln(III) ions were recorded (Figure 4a) under the same conditions (λex = 320 nm; ex/em slit 5/1.5 nm; data interval 1.0 nm; average time 0.10 s; PMT voltage 800 V).The most intensive emission was detected for TbBDC, followed by EuBDC.Emission from SmBDC and DyBDC was also present, as can be seen from the normalized spectra (Figure S2), but obviously, terephthalic acid is not a good sensitizer of their luminescence, observed as well in [11].A possible explanation is the small energy gap possessed by Dy(III) and Sm(III) [31], which favors nonradiative deactivation, especially in the presence of coordinated water molecules.The energy of the lowest triplet state of terephthalic acid, 23,530 cm −1 [11], happens to be suitable for the energy gap between the emitting level 5 D 4 of Tb(III) [32]; therefore, good luminescence was detected for TbBDC.As a difference, a lower emission by EuBDC in comparison to that by TbBDC was noticed.To ensure the lack/existence of self-quenching effects, the luminescence of the samples in a mixture with BaSO 4 was recorded (LnBDC in BaSO 4 5 wt%).It was clearly observed (Figure 4b) that the emissions from TbBDC and EuBDC now were of almost equal intensity.This observation is evidence of the self-quenching effect, significantly influencing the EuBDC emission.Following the results observed, subsequent measurements and experiments on sensor properties were focused mainly on Tb(III) and Eu(III) samples.Lifetime measurements in the solid state and in a water suspension also demonstrated longer lifetimes for TbBDC, both in the solid state and in the water suspension (Table 1).The decay curves were fi ed monoexponentially.The values obtained for TbBDC and EuBDC are in agreement with the literature data for this composition [11].No significant difference was observed when the lifetimes were measured in mixtures with BaSO4.

Sensor Properties
As mentioned before, the experiments for sensor properties were performed only with EuBDC and TbBDC samples because of their more intense luminescence.As the specific surface area and the pore size are important parameters for the sensor performance of materials, N2 adsorption-desorption analysis of TbBDC and EuBDC was performed.The obtained isotherms (Figure S3) were of type IV, with an H3-type hysteresis loop according to the IUPAC classification [33].This indicated weak adsorbent-adsorbate interactions, and it is typical for nonporous or microporous solids, which is in good agreement with the literature data for these MOFs.The calculated specific surface area, the average pore volume, and the total pore volume are summarized in Table S3.The calculated specific area was 14. 60 and 14.75 m 2 /g for TbBDC and EuBDC, respectively.The Lifetime measurements in the solid state and in a water suspension also demonstrated longer lifetimes for TbBDC, both in the solid state and in the water suspension (Table 1).The decay curves were fitted monoexponentially.The values obtained for TbBDC and EuBDC are in agreement with the literature data for this composition [11].No significant difference was observed when the lifetimes were measured in mixtures with BaSO 4 .

Sensor Properties
As mentioned before, the experiments for sensor properties were performed only with EuBDC and TbBDC samples because of their more intense luminescence.As the specific surface area and the pore size are important parameters for the sensor performance of materials, N 2 adsorption-desorption analysis of TbBDC and EuBDC was performed.The obtained isotherms (Figure S3) were of type IV, with an H3-type hysteresis loop according to the IUPAC classification [33].This indicated weak adsorbent-adsorbate interactions, and it is typical for nonporous or microporous solids, which is in good agreement with the literature data for these MOFs.The calculated specific surface area, the average pore volume, and the total pore volume are summarized in Table S3.The calculated specific area was 14. 60 and 14.75 m 2 /g for TbBDC and EuBDC, respectively.The values obtained are significantly higher than the literature data for the same structure [34], confirming that the synthesis conditions and resulting morphology play a significant role in the sensor's properties and performance ability.
Preliminary experiments in order to determine the best concentration of the samples in water suspensions were performed (Figure S4).As a result, the concentration of 0.5 mg/mL for the samples was selected for further research.This concentration ensures suspension stability and helps to avoid self-quenching of Ln(III) ions.

Stability of the Water Suspensions of the Samples
Luminescence was recorded, both of freshly prepared and of 3-week-aged suspensions (Figure 5a,b).First, the suspension was centrifugated.Next, the sample was dried.Finally, the phase homogeneity was determined by powder XRD (Figure 5c,d).With this procedure, the stability in water and after multiple ultrasound treatments was evaluated.
Molecules 2024, 29, x FOR PEER REVIEW 7 of 23 confirming that the synthesis conditions and resulting morphology play a significant role in the sensor's properties and performance ability.Preliminary experiments in order to determine the best concentration of the samples in water suspensions were performed (Figure S4).As a result, the concentration of 0.5 mg/mL for the samples was selected for further research.This concentration ensures suspension stability and helps to avoid self-quenching of Ln(III) ions.

Stability of the Water Suspensions of the Samples
Luminescence was recorded, both of freshly prepared and of 3-week-aged suspensions (Figure 5a,b).First, the suspension was centrifugated.Next, the sample was dried.Finally, the phase homogeneity was determined by powder XRD (Figure 5c,d).With this procedure, the stability in water and after multiple ultrasound treatments was evaluated.The results confirmed that both EuBDC and TbBDC samples are stable in water for at least 3 weeks.Luminescence was kept stable, and powder X-ray diffraction showed no change in the sample phase composition.

Behavior in Different Solvents
Suspensions in different solvents were prepared, and their luminescence was measured according to the procedure described in Section 3 (Materials and Methods).Both samples were sensitive to acetone, and the luminescence was fully quenched in that solvent (Figure 6), but the luminescence recovered after the removal of acetone (Figure S5).Although some studies have focused on sensing acetone in water [35][36][37][38], it is not considered a water pollutant, due to its volatility.The results confirmed that both EuBDC and TbBDC samples are stable in water for at least 3 weeks.Luminescence was kept stable, and powder X-ray diffraction showed no change in the sample phase composition.

Behavior in Different Solvents
Suspensions in different solvents were prepared, and their luminescence was measured according to the procedure described in Section 3 (Materials and Methods).Both samples were sensitive to acetone, and the luminescence was fully quenched in that solvent (Figure 6), but the luminescence recovered after the removal of acetone (Figure S5).Although some studies have focused on sensing acetone in water [35][36][37][38], it is not considered a water pollutant, due to its volatility.

Behavior in Media with Different Acidity Levels
An important property of potential sensors is their behavior in media with different acidity levels.The pH value of natural waters depends on many variables, but usually, waste waters from mines have a pH of about 2 to 3; swamps, 4 to 6; groundwaters, 5 to 7; rivers, 7-8; fresh lakes, 7-9.5; and oceans, 8-8.5 [39].So, obviously, it is crucial to know the sensor behavior in these pH ranges.
Measurements were performed according to the procedure described in Section 3 (Materials and Methods).From Figure 7, it is seen that both EuBDC and TbBDC behave similarly and have stable luminescence in the pH range of 4 to 9. In both cases, it was observed that there was a decrease in the luminescence at a pH of about 3 and about 10 and almost full loss of luminescence at a pH below 3 and over 10.Such a drastic loss of luminescence is most likely due to the destruction of the MOF.This was additionally confirmed with PXRD of the TbBDC sample at pH 1.5 and pH 11.90 (Figure S6).At low pH, reflections from H2BDC were observed, which is a clear indication of the destruction of the original MOF.At high pH, no crystal phase could be observed, suggesting a destruction process and the presence of the amorphous hydroxide of Ln(III).Nevertheless, both samples demonstrated a good working range for drinking waters, and it is worth continuing the tests.

Behavior in the Presence of Different Cations and Anions
Emissions from the samples were measured under the same conditions, and to detect sensor properties, the maximum emission wavelength was applied, at 616 and 547 nm for

Behavior in Media with Different Acidity Levels
An important property of potential sensors is their behavior in media with different acidity levels.The pH value of natural waters depends on many variables, but usually, waste waters from mines have a pH of about 2 to 3; swamps, 4 to 6; groundwaters, 5 to 7; rivers, 7-8; fresh lakes, 7-9.5; and oceans, 8-8.5 [39].So, obviously, it is crucial to know the sensor behavior in these pH ranges.
Measurements were performed according to the procedure described in Section 3 (Materials and Methods).From Figure 7, it is seen that both EuBDC and TbBDC behave similarly and have stable luminescence in the pH range of 4 to 9. In both cases, it was observed that there was a decrease in the luminescence at a pH of about 3 and about 10 and almost full loss of luminescence at a pH below 3 and over 10.Such a drastic loss of luminescence is most likely due to the destruction of the MOF.This was additionally confirmed with PXRD of the TbBDC sample at pH 1.5 and pH 11.90 (Figure S6).At low pH, reflections from H 2 BDC were observed, which is a clear indication of the destruction of the original MOF.At high pH, no crystal phase could be observed, suggesting a destruction process and the presence of the amorphous hydroxide of Ln(III).Nevertheless, both samples demonstrated a good working range for drinking waters, and it is worth continuing the tests.

Behavior in Media with Different Acidity Levels
An important property of potential sensors is their behavior in media with different acidity levels.The pH value of natural waters depends on many variables, but usually, waste waters from mines have a pH of about 2 to 3; swamps, 4 to 6; groundwaters, 5 to 7; rivers, 7-8; fresh lakes, 7-9.5; and oceans, 8-8.5 [39].So, obviously, it is crucial to know the sensor behavior in these pH ranges.
Measurements were performed according to the procedure described in Section 3 (Materials and Methods).From Figure 7, it is seen that both EuBDC and TbBDC behave similarly and have stable luminescence in the pH range of 4 to 9. In both cases, it was observed that there was a decrease in the luminescence at a pH of about 3 and about 10 and almost full loss of luminescence at a pH below 3 and over 10.Such a drastic loss of luminescence is most likely due to the destruction of the MOF.This was additionally confirmed with PXRD of the TbBDC sample at pH 1.5 and pH 11.90 (Figure S6).At low pH, reflections from H2BDC were observed, which is a clear indication of the destruction of the original MOF.At high pH, no crystal phase could be observed, suggesting a destruction process and the presence of the amorphous hydroxide of Ln(III).Nevertheless, both samples demonstrated a good working range for drinking waters, and it is worth continuing the tests.

Behavior in the Presence of Different Cations and Anions
Emissions from the samples were measured under the same conditions, and to detect sensor properties, the maximum emission wavelength was applied, at 616 and 547 nm for

Behavior in the Presence of Different Cations and Anions
Emissions from the samples were measured under the same conditions, and to detect sensor properties, the maximum emission wavelength was applied, at 616 and 547 nm for EuBDC and TbBDC, respectively.The procedure is described in Section 3 (Methods and Materials).
The sensor properties of both EuBDC and TbBDC were tested for 16 different cations (Figure 8).Based on the emission registered, the samples showed the highest sensitivity to Fe(III), followed by Ag(I).Sensitivity to Cr(III) differed essentially, and EuBDC can be used as a sensor for Cr(III).The results with anions were promising, too (Figure 9 EuBDC and TbBDC, respectively.The procedure is described in Section 3 (Methods and Materials).
The sensor properties of both EuBDC and TbBDC were tested for 16 different cations (Figure 8).Based on the emission registered, the samples showed the highest sensitivity to Fe(III), followed by Ag(I).Sensitivity to Cr(III) differed essentially, and EuBDC can be used as a sensor for Cr(III).The results with anions were promising, too (Figure 9); namely, (i) both samples were sensitive to MnO4 −  The pH levels of the solutions of the ions were measured in order to exclude the influence of the acidity of the environment (Table S4).As data on the potential health effects of manganese remain uncertain, particularly relating to the form of manganese that may be of concern, and it was difficult to determine a suitable health-based value at this time [40], we did not perform experiments with it.As long as the oxalate ions form lowsolubility products with cations usually present in water, they are not considered a threat.The following sections present research results with the ions of Ag(I), Cr(III), Fe(III), and Cr(VI).

Silver(I) Sensitivity of EuBDC and of TbBDC
Average silver concentrations in natural waters according to the World Health Organization are 0.2-0.3µg/L [41].Water treated with silver may have ion levels of 50 µg/L or higher.Higher levels of silver ions, up to 0.1 mg/L (a concentration that gives a EuBDC and TbBDC, respectively.The procedure is described in Section 3 (Methods and Materials).
The sensor properties of both EuBDC and TbBDC were tested for 16 different cations (Figure 8).Based on the emission registered, the samples showed the highest sensitivity to Fe(III), followed by Ag(I).Sensitivity to Cr(III) differed essentially, and EuBDC can be used as a sensor for Cr(III).The results with anions were promising, too (Figure 9); namely, (i) both samples were sensitive to MnO4 −  The pH levels of the solutions of the ions were measured in order to exclude the influence of the acidity of the environment (Table S4).As data on the potential health effects of manganese remain uncertain, particularly relating to the form of manganese that may be of concern, and it was difficult to determine a suitable health-based value at this time [40], we did not perform experiments with it.As long as the oxalate ions form lowsolubility products with cations usually present in water, they are not considered a threat.The following sections present research results with the ions of Ag(I), Cr(III), Fe(III), and Cr(VI).

Silver(I) Sensitivity of EuBDC and of TbBDC
Average silver concentrations in natural waters according to the World Health Organization are 0.2-0.3µg/L [41].Water treated with silver may have ion levels of 50 µg/L or higher.Higher levels of silver ions, up to 0.1 mg/L (a concentration that gives a The pH levels of the solutions of the ions were measured in order to exclude the influence of the acidity of the environment (Table S4).As data on the potential health effects of manganese remain uncertain, particularly relating to the form of manganese that may be of concern, and it was difficult to determine a suitable health-based value at this time [40], we did not perform experiments with it.As long as the oxalate ions form low-solubility products with cations usually present in water, they are not considered a threat.The following sections present research results with the ions of Ag(I), Cr(III), Fe(III), and Cr(VI).

Silver(I) Sensitivity of EuBDC and of TbBDC
Average silver concentrations in natural waters according to the World Health Organization are 0.2-0.3µg/L [41].Water treated with silver may have ion levels of 50 µg/L or higher.Higher levels of silver ions, up to 0.1 mg/L (a concentration that gives a total dose over 70 years of half the human no-observed-adverse-effect level (NOAEL) of 10 g), could then be tolerated without risk to health [41].So, silver is an element of interest, and a concentration above 9.27×10 −7 mol/L is considered dangerous for humans, and further tests will be performed.The procedure is explained in Section 3.
A gradual decrease in luminescence was observed with an increase in the concentration of Ag(I) (Figure 10).By plotting the intensity in the absence of a quencher versus the intensity in the presence of a quencher (I 0 /I) to the concentration of Ag(I) ions in both MOFs, exponential curves were obtained (Figure 11).In Section 3.5.4are described all the equations used for the discussion of the following results.Equation ( 7) was used to describe the data from Figure 11.
total dose over 70 years of half the human no-observed-adverse-effect level (NOAEL) of 10 g), could then be tolerated without risk to health [41].So, silver is an element of interest, and a concentration above 9.27×10 −7 mol/L is considered dangerous for humans, and further tests will be performed.The procedure is explained in Section 3.
A gradual decrease in luminescence was observed with an increase in the concentration of Ag(I) (Figure 10).By plo ing the intensity in the absence of a quencher versus the intensity in the presence of a quencher (I0/I) to the concentration of Ag(I) ions in both MOFs, exponential curves were obtained (Figure 11).In Section 3.5.4are described all the equations used for the discussion of the following results.Equation ( 7) was used to describe the data from Figure 11.From Figure 11a, for EuBDC with Ag(I), exponential fi ing of I0/I = 0.00123e 5.61691[Q] + 0.8033 was obtained.The Stern-Volmer constant Ksv was calculated to be 6.908 M −1 (R 2 = 0.99124).For TbBDC (Figure 11b), I0/I = 0.0037e 5.30066[Q] + 1.30927, and Ksv was calculated to be 19.61M −1 (R 2 = 0.99867).Both values for Ksv were low, but one has to keep in mind that there are no data specifically for the Ksv for Ag(I) when MOF materials are used as sensors.
When solutions with concentrations up to 0.8 mM of Ag(I) were tested, a linear dependence with much higher values of Ksv (Figure 12a) was observed.total dose over 70 years of half the human no-observed-adverse-effect level (NOAEL) of 10 g), could then be tolerated without risk to health [41].So, silver is an element of interest, and a concentration above 9.27×10 −7 mol/L is considered dangerous for humans, and further tests will be performed.The procedure is explained in Section 3.
A gradual decrease in luminescence was observed with an increase in the concentration of Ag(I) (Figure 10).By plo ing the intensity in the absence of a quencher versus the intensity in the presence of a quencher (I0/I) to the concentration of Ag(I) ions in both MOFs, exponential curves were obtained (Figure 11).In Section 3.5.4are described all the equations used for the discussion of the following results.Equation ( 7) was used to describe the data from Figure 11.From Figure 11a, for EuBDC with Ag(I), exponential fi ing of I0/I = 0.00123e 5.61691[Q] + 0.8033 was obtained.The Stern-Volmer constant Ksv was calculated to be 6.908 M −1 (R 2 = 0.99124).For TbBDC (Figure 11b), I0/I = 0.0037e 5.30066[Q] + 1.30927, and Ksv was calculated to be 19.61M −1 (R 2 = 0.99867).Both values for Ksv were low, but one has to keep in mind that there are no data specifically for the Ksv for Ag(I) when MOF materials are used as sensors.
When solutions with concentrations up to 0.8 mM of Ag(I) were tested, a linear dependence with much higher values of Ksv (Figure 12a) was observed.From Figure 11a, for EuBDC with Ag(I), exponential fitting of I 0 /I = 0.00123e 5.61691[Q] + 0.8033 was obtained.The Stern-Volmer constant K sv was calculated to be 6.908 M −1 (R 2 = 0.99124).For TbBDC (Figure 11b), I 0 /I = 0.0037e 5.30066[Q] + 1.30927, and K sv was calculated to be 19.61M −1 (R 2 = 0.99867).Both values for K sv were low, but one has to keep in mind that there are no data specifically for the K sv for Ag(I) when MOF materials are used as sensors.
When solutions with concentrations up to 0.8 mM of Ag(I) were tested, a linear dependence with much higher values of K sv (Figure 12a) was observed.
The values obtained for EuBDC were K sv = 2911 M −1 and R 2 = 0.99957 and for TbBDC were K sv = 8322 M −1 and R 2 = 0.99302.These values were much higher compared to those calculated from the exponential fit, suggesting that both materials can be used as sensors only at low concentrations.It is clear that TbBDC performs much better than EuBDC, with a higher value for Ksv and a lower value for LOD (88 µM for TbBDC compared to 104 µM for EuBDC) (Table S5).The LOD is 3σ/slope, where σ is the standard deviation of the blank sample measured 10 times, and the slope is taken from the intensity-versus-concentration plot in the linear region.The values obtained for EuBDC were Кsv = 2911 M −1 and R 2 = 0.99957 and for TbBDC were Кsv = 8322 M −1 and R 2 = 0.99302.These values were much higher compared to those calculated from the exponential fit, suggesting that both materials can be used as sensors only at low concentrations.It is clear that TbBDC performs much be er than EuBDC, with a higher value for Ksv and a lower value for LOD (88 µM for TbBDC compared to 104 µM for EuBDC) (Table S5).The LOD is 3σ/slope, where σ is the standard deviation of the blank sample measured 10 times, and the slope is taken from the intensity-versus-concentration plot in the linear region.
When the concentration of silver ions was high enough to quench almost 100% of the luminescence, emission from the linker was clearly observed (Figure 13).All a empts to recover the luminescence after washing the sample were unsuccessful.This may suggest a more complex character of the quenching and explain the high exponential dependence at higher concentrations and unusual Ksv values.It can be suggested that at low concentrations, dynamic quenching plays a major role, and at a concentration higher than 0.8 mM, static quenching called "sphere of action" is also present.Moreover, as the luminescence did not recover after full quenching, we again explored PXRD, and pa erns of the silver MOF [42] with terephthalic acid were observed (Figure S6).Obviously, partial destruction of the original MOF also plays a role and explains the unusual Stern-Volmer dependence.

Chromium (III) Sensitivity of EuBDC
Chromium(III) was tested only with EuBDC (Figure 14a) as EuBDC is more sensitive to it (see Figure 8).A guideline value (GV) of 50 µg/L has been proposed for the total When the concentration of silver ions was high enough to quench almost 100% of the luminescence, emission from the linker was clearly observed (Figure 13).All attempts to recover the luminescence after washing the sample were unsuccessful.This may suggest a more complex character of the quenching and explain the high exponential dependence at higher concentrations and unusual K sv values.The values obtained for EuBDC were Кsv = 2911 M −1 and R 2 = 0.99957 and for TbBDC were Кsv = 8322 M −1 and R 2 = 0.99302.These values were much higher compared to those calculated from the exponential fit, suggesting that both materials can be used as sensors only at low concentrations.It is clear that TbBDC performs much be er than EuBDC, with a higher value for Ksv and a lower value for LOD (88 µM for TbBDC compared to 104 µM for EuBDC) (Table S5).The LOD is 3σ/slope, where σ is the standard deviation of the blank sample measured 10 times, and the slope is taken from the intensity-versus-concentration plot in the linear region.
When the concentration of silver ions was high enough to quench almost 100% of the luminescence, emission from the linker was clearly observed (Figure 13).All a empts to recover the luminescence after washing the sample were unsuccessful.This may suggest a more complex character of the quenching and explain the high exponential dependence at higher concentrations and unusual Ksv values.It can be suggested that at low concentrations, dynamic quenching plays a major role, and at a concentration higher than 0.8 mM, static quenching called "sphere of action" is also present.Moreover, as the luminescence did not recover after full quenching, we again explored PXRD, and pa erns of the silver MOF [42] with terephthalic acid were observed (Figure S6).Obviously, partial destruction of the original MOF also plays a role and explains the unusual Stern-Volmer dependence.

Chromium (III) Sensitivity of EuBDC
Chromium(III) was tested only with EuBDC (Figure 14a) as EuBDC is more sensitive to it (see Figure 8).A guideline value (GV) of 50 µg/L has been proposed for the total It can be suggested that at low concentrations, dynamic quenching plays a major role, and at a concentration higher than 0.8 mM, static quenching called "sphere of action" is also present.Moreover, as the luminescence did not recover after full quenching, we again explored PXRD, and patterns of the silver MOF [42] with terephthalic acid were observed (Figure S6).Obviously, partial destruction of the original MOF also plays a role and explains the unusual Stern-Volmer dependence.

Chromium (III) Sensitivity of EuBDC
Chromium(III) was tested only with EuBDC (Figure 14a) as EuBDC is more sensitive to it (see Figure 8).A guideline value (GV) of 50 µg/L has been proposed for the total chromium content based on achievability by current treatment technologies, measurability by analytical methods, and toxicology [43].The risk assessment for chromium in drinking water is based on recent high-quality data from chronic drinking-water carcinogenicity and mode-of-action studies for Cr(III) and Cr(VI).As chromium is usually found in drinking water at an average concentration of 1 µg/L, which is below the GV, in general, the monitoring and inclusion of Cr in drinking-water regulations and standards would only be necessary if there were indications that a problem might exist [43].
chromium in drinking water is based on recent high-quality data from chronic drinkingwater carcinogenicity and mode-of-action studies for Cr(III) and Cr(VI).As chromium is usually found in drinking water at an average concentration of 1 µg/L, which is below the GV, in general, the monitoring and inclusion of Cr in drinking-water regulations and standards would only be necessary if there were indications that a problem might exist [43].Again, an exponential curve was observed with fi ing I0/I = 0.00106e 2.60329[Q] + 1.17343 (Figure 14b).The value of Ksv was calculated to be 2.76 M −1 (R 2 = 0.99975).This is similar behavior to the one observed in the case of Ag(I).Linear dependency at lower concentrations of up to 2.4 mM (Figure 15) and a Ksv value of 3440 M −1 was observed, suggesting again that this sensor is appropriate only for low concentrations of Cr(III).In this case, as well as with Ag(I), after quenching, full recovery of luminescence was not possible.Most likely, again, a destruction process was involved, so the application of these materials as sensors for Ag(I) and Cr(III) will be difficult and will limit it in a narrow concentration range.Moreover, the LODs calculated from the linear dependence for both materials and ions were high (see Table S5).However, this unusual form of the exponential curve can be used to recognize the influence of MOF destruction processes.It is also important to know the behavior of a given material toward any ion potentially present in water in order to fully appreciate its capabilities.Again, an exponential curve was observed with fitting I 0 /I = 0.00106e 2.60329[Q] + 1.17343 (Figure 14b).The value of K sv was calculated to be 2.76 M −1 (R 2 = 0.99975).This is similar behavior to the one observed in the case of Ag(I).Linear dependency at lower concentrations of up to 2.4 mM (Figure 15) and a Ksv value of 3440 M −1 was observed, suggesting again that this sensor is appropriate only for low concentrations of Cr(III).In this case, as well as with Ag(I), after quenching, full recovery of luminescence was not possible.Most likely, again, a destruction process was involved, so the application of these materials as sensors for Ag(I) and Cr(III) will be difficult and will limit it in a narrow concentration range.Moreover, the LODs calculated from the linear dependence for both materials and ions were high (see Table S5).However, this unusual form of the exponential curve can be used to recognize the influence of MOF destruction processes.It is also important to know the behavior of a given material toward any ion potentially present in water in order to fully appreciate its capabilities.
chromium in drinking water is based on recent high-quality data from chronic drinkingwater carcinogenicity and mode-of-action studies for Cr(III) and Cr(VI).As chromium is usually found in drinking water at an average concentration of 1 µg/L, which is below the GV, in general, the monitoring and inclusion of Cr in drinking-water regulations and standards would only be necessary if there were indications that a problem might exist [43].Again, an exponential curve was observed with fi ing I0/I = 0.00106e 2.60329[Q] + 1.17343 (Figure 14b).The value of Ksv was calculated to be 2.76 M −1 (R 2 = 0.99975).This is similar behavior to the one observed in the case of Ag(I).Linear dependency at lower concentrations of up to 2.4 mM (Figure 15) and a Ksv value of 3440 M −1 was observed, suggesting again that this sensor is appropriate only for low concentrations of Cr(III).In this case, as well as with Ag(I), after quenching, full recovery of luminescence was not possible.Most likely, again, a destruction process was involved, so the application of these materials as sensors for Ag(I) and Cr(III) will be difficult and will limit it in a narrow concentration range.Moreover, the LODs calculated from the linear dependence for both materials and ions were high (see Table S5).However, this unusual form of the exponential curve can be used to recognize the influence of MOF destruction processes.It is also important to know the behavior of a given material toward any ion potentially present in water in order to fully appreciate its capabilities.

Iron (III) Sensitivity of TbBDC
According to the WHO [44], the median iron concentration in rivers has been reported to be 0.7 mg/L.In anaerobic groundwater where iron is in the form of iron(II), concentrations will usually be 0.5-10 mg/L, but concentrations up to 50 mg/L can sometimes be found as well.Concentrations of iron in drinking waters are normally less than 0.3 mg/L but may be higher in countries where various iron salts are used as coagulating agents in water treatment plants and where cast iron, steel, and galvanized iron pipes are used for water distribution.Taste is not usually noticeable at iron concentrations below 0.3 mg/L, although turbidity and color may develop in piped systems at levels above 0.05-0.1 mg/L.Laundry and sanitaryware will get stained at iron concentrations above 0.3 mg/L.Allocation of 10% of the provisional maximum tolerable daily intake of drinking water provides a value of about 2 mg/L, which does not present a hazard to health.The taste and appearance of drinking water will usually be affected below this level, although iron concentrations of 1-3 mg/L can be acceptable for people drinking anaerobic well water [44].Apparently, this cation is of great interest, as quite a lot of studies have investigated Ln-MOFs as sensors of Fe(III) [21,[45][46][47][48][49][50][51][52].
A plot of the data from a luminescent sensor experiment with Fe(III) can be seen in Figure 16a.
concentrations below 0.3 mg/L, although turbidity and color may develop in piped systems at levels above 0.05-0.1 mg/L.Laundry and sanitaryware will get stained at iron concentrations above 0.3 mg/L.Allocation of 10% of the provisional maximum tolerable daily intake of drinking water provides a value of about 2 mg/L, which does not present a hazard to health.The taste and appearance of drinking water will usually be affected below this level, although iron concentrations of 1-3 mg/L can be acceptable for people drinking anaerobic well water [44].Apparently, this cation is of great interest, as quite a lot of studies have investigated Ln-MOFs as sensors of Fe(III) [21,[45][46][47][48][49][50][51][52].
A plot of the data from a luminescent sensor experiment with Fe(III) can be seen in Figure 16a.As discussed in Section 3.5.4,when both static quenching and dynamic quenching were combined, we observed both quenching by collisions and quenching by complex formation with the same quencher.The Stern-Volmer equation is a second-order polynomial curve (Equation ( 3)).The fi ing was good, with R 2 = 0.9995 (Figure 16a).
During the measurement, the lifetime was also determined (Figure 16b) for each concentration of the quencher.We observed a small value for the slope, suggesting that the dynamic quenching constant is low and, obviously, we have bigger static quenching.We can see from Figure 16b that dynamic quenching played a role again at low concentrations and above 0.4 mM.We can use the modified Equation (3) to allow a graphical separation of KS and KD for the apparent quenching constant (Equations ( 4) and ( 5)) shown in Figure 17.As discussed in Section 3.5.4,when both static quenching and dynamic quenching were combined, we observed both quenching by collisions and quenching by complex formation with the same quencher.The Stern-Volmer equation is a second-order polynomial curve (Equation ( 3)).The fitting was good, with R 2 = 0.9995 (Figure 16a).
During the measurement, the lifetime was also determined (Figure 16b) for each concentration of the quencher.We observed a small value for the slope, suggesting that the dynamic quenching constant is low and, obviously, we have bigger static quenching.We can see from Figure 16b that dynamic quenching played a role again at low concentrations and above 0.4 mM.We can use the modified Equation (3) to allow a graphical separation of K S and K D for the apparent quenching constant (Equations ( 4) and ( 5)) shown in Figure 17.The possible value for KS was 4777 or 881 M −1 .Lifetime data (Figure 16b) suggested that the higher value is more reasonable for a static quenching constant.
The data could be fi ed exponentially, too, with a similar value of R 2 of 0.99917 (Figure 18).The possible value for K S was 4777 or 881 M −1 .Lifetime data (Figure 16b) suggested that the higher value is more reasonable for a static quenching constant.
The data could be fitted exponentially, too, with a similar value of R 2 of 0.99917 (Figure 18).When we used exponential fitting, we could determine K sv (see Equation ( 5)), so the value was 6903 M −1 .This value is in good agreement with literature data, where values from 1000 M −1 to 13,000 M −1 can be found for Fe(III) sensing [21,[45][46][47][48][49][50][51][52].Of course, data can be fitted linearly up to concentrations of 1.0 mM, with reasonable values of R 2 = 0.9939 and K sv = 8924 M −1 (Figure S8).The LOD was 32.5 µM, which is much better than that calculated for Ag(I) and Cr(III).A comparison of the types of data manipulations is summarized in Table S5.The possible value for KS was 4777 or 881 M −1 .Lifetime data (Figure 16b) suggested that the higher value is more reasonable for a static quenching constant.
The data could be fi ed exponentially, too, with a similar value of R 2 of 0.99917 (Figure 18).When we used exponential fi ing, we could determine Ksv (see Equation ( 5)), so the value was 6903 M −1 .This value is in good agreement with literature data, where values from 1000 M −1 to 13,000 M −1 can be found for Fe(III) sensing [21,[45][46][47][48][49][50][51][52].Of course, data can be fi ed linearly up to concentrations of 1.0 mM, with reasonable values of R 2 = 0.9939 and Ksv = 8924 M −1 (Figure S8).The LOD was 32.5 µM, which is much be er than that calculated for Ag(I) and Cr(III).A comparison of the types of data manipulations is summarized in Table S5.

Chromium (VI) sensitivity of TbBDC
As discussed already, chromium is explored in water as the total for both Cr(III) and Cr(VI).Interestingly, only EuBDC demonstrated sensitivity to Cr(III), which can be used as a tool to determine different forms of chromium in water, as for Cr(VI), both EuBDC and TbBDC were sensitive, and tests were performed with the be er-luminescent TbBDC.
Again, polynomic fit and exponential fit can be applied to the data, both with high R 2 (Figure 19), but in this case, we could not obtain real solutions from the polynomic fit when using Equations ( 4) and (5) (Figure S9).Apparently, the value from the intercept is mainly from static quenching.Lifetime measurements (Figure 20) suggested independence of the lifetime from the concentration, as the slope was low and we observed dynamic quenching only at low concentrations.Most likely, static quenching plays a major role in both types: (i) the formation of a nonfluorescent ground state confirmed by the independence of the lifetime and (ii) "sphere of action", confirmed by the exponential fit.

Chromium (VI) sensitivity of TbBDC
As discussed already, chromium is explored in water as the total for both Cr(III) and Cr(VI).Interestingly, only EuBDC demonstrated sensitivity to Cr(III), which can be used as a tool to determine different forms of chromium in water, as for Cr(VI), both EuBDC and TbBDC were sensitive, and tests were performed with the better-luminescent TbBDC.
Again, polynomic fit and exponential fit can be applied to the data, both with high R 2 (Figure 19), but in this case, we could not obtain real solutions from the polynomic fit when using Equations ( 4) and ( 5) (Figure S9).Apparently, the value from the intercept is mainly from static quenching.Lifetime measurements (Figure 20) suggested independence of the lifetime from the concentration, as the slope was low and we observed dynamic quenching only at low concentrations.Most likely, static quenching plays a major role in both types: (i) the formation of a nonfluorescent ground state confirmed by the independence of the lifetime and (ii) "sphere of action", confirmed by the exponential fit.Furthermore, the calculated Ksv value from the exponential fit of the data was 2093 M −1 .This value is also in good agreement with literature data [46,[53][54][55].Linear fit (Figure S10) gives a Ksv value of 2749 M −1 and an LOD value of 49.5 µM, suggesting there is good potential of this material as a sensor for Cr(VI).It is worth mentioning that the different type of exponential fi ing for Cr(III) (see Figure 14b) is one more way to separate the two oxidation forms when tested.Furthermore, the calculated Ksv value from the exponential fit of the data was 2093 M −1 .This value is also in good agreement with literature data [46,[53][54][55].Linear fit (Figure S10) gives a Ksv value of 2749 M −1 and an LOD value of 49.5 µM, suggesting there is good potential of this material as a sensor for Cr(VI).It is worth mentioning that the different type of exponential fi ing for Cr(III) (see Figure 14b) is one more way to separate the two Furthermore, the calculated K sv value from the exponential fit of the data was 2093 M −1 .This value is also in good agreement with literature data [46,[53][54][55].Linear fit (Figure S10) gives a K sv value of 2749 M −1 and an LOD value of 49.5 µM, suggesting there is good potential of this material as a sensor for Cr(VI).It is worth mentioning that the different type of exponential fitting for Cr(III) (see Figure 14b) is one more way to separate the two oxidation forms when tested.2.5.9.Possible Quenching Mechanisms A more detailed discussion of the mechanisms of luminescence quenching in the presence of acetone, Ag(I), Cr(III), Fe(III), and CrO 4 2− /Cr 2 O 7 2− is presented in this section.A possible mechanism of quenching with acetone is Förster resonance energy transfer, i.e., a nonradiative transfer of energy from a donor to an acceptor molecule (observed if the acceptor molecule possesses high-energy vibrational states, e.g., it is an organic molecule with functional groups such as -OH, -CN, and -NO 2 ) [37].After the removal of acetone, full recovery of the luminescence is observed (Figure S5).Acetone has an observable absorption in the 225-325 nm region, while the other solvents do not possess an absorption band at 320 nm [56].Based on this, energy transfer between the ligand and acetone can be suggested, indicating a sort of competitiveness between the compound excitation and the acetone absorption.The latter causes a decrease in the luminescence intensity.As previously mentioned, acetone is not considered a water pollutant, and experiments with different concentrations were not performed.In spite of that, we considered the elucidation of the quenching mechanism, as well as of the luminescence recovering after acetone removal, an important move for further experiments.
Regarding the change in the luminescence of MOFs caused by the metal ions, four different mechanisms have been reported, taking into consideration (i) a weak interaction between the metal ions and the free Lewis basic sites within the organic ligands of the MOF, (ii) an ion exchange between the central metal ion and the targeted ions, (iii) destruction of the framework, and (iv) absorption of excitation light, FRET, and other excited-state processes [57].
In the case of Ag(I) and Cr(III) quenching, Stern-Volmer plots of the data showed similarity, and a recovery of the luminescence was not possible.This, along with the evidence that a different MOF formation was observed (Figure 21) and no overlap of the absorption of these ions with the excitation of the LnBDC was observed (Figure 21), provides a reason to exclude as an option mechanism (iv) mentioned before but confirms that the destruction of the initial MOF (iii) is the most important effect.Regarding the change in the luminescence of MOFs caused by the metal ions, four different mechanisms have been reported, taking into consideration (i) a weak interaction between the metal ions and the free Lewis basic sites within the organic ligands of the MOF, (ii) an ion exchange between the central metal ion and the targeted ions, (iii) destruction of the framework, and (iv) absorption of excitation light, FRET, and other excited-state processes [57].
In the case of Ag(I) and Cr(III) quenching, Stern-Volmer plots of the data showed similarity , and a recovery of the luminescence was not possible.This, along with the evidence that a different MOF formation was observed (Figure 21) and no overlap of the absorption of these ions with the excitation of the LnBDC was observed (Figure 21), provides a reason to exclude as an option mechanism (iv) mentioned before but confirms that the destruction of the initial MOF (iii) is the most important effect.In the case of Fe(III) and CrO4 2−/ Cr2O7 2 − quenching, we have to consider that the luminescence of Ln-MOFs mainly suffers from the "antenna effect", i.e., the ligands efficiently absorb and transfer light to the luminescent central lanthanide ions.As shown in Figure 21, the UV-VIS absorption spectra of Fe(III) and CrO4 2−/ Cr2O7 2− emerged as strong absorption bands in the range of 200-350 nm for Fe(III) and 260-400 nm for CrO4 2−/ Cr2O7 2− , while the excitation of LnBDC was at 320 nm.These facts imply that Fe(III) and CrO4 2−/ Cr2O7 2 could drastically absorb the energy of the excitation, reducing the efficiency of energy transfer from the ligand to the lanthanide ions and, by that, definitely induce the luminescence-quenching effect.All these suggest a Förster resonance energy transfer again.the efficiency of energy transfer from the ligand to the lanthanide ions and, by that, definitely induce the luminescence-quenching effect.All these suggest a Förster resonance energy transfer again.

Materials Used
All the chemicals for the experiments were analytical grade.Terephthalic acid was procured from Thermo Scientific™, Waltham, MA, USA.LnCl IR analysis (see Figure S11) additionally confirmed that the samples were isostructural, and there was a coordination to H 2 BDC.The vibrations assignment of the free terephthalic acid was done according to [58].

Single-Crystal Growth of DyBDC-SC
A single crystal of the powdered sample with the composition [Ln 2 (BDC) 3 (H 2 O) 4 ] ∞ was obtained under solvothermal conditions.DyCl 3 •nH 2 O (0.1 mmol) and H 2 BCD (0.05 mmol) were dissolved in 11 mL of acetonitrile/water mixture (1:1.75 volume ratio), and 0.3 mL of 1 mol/L of HCl was added to the solution.The mixture was placed in a 20 mL Teflon-lined stainless-steel reactor and kept at 140 • C for 72 h, with a 15 • C/h step of increasing temperature and a 5 • C/h step of cooling.After cool-down, a small number of crystals were found suitable to be measured with single-crystal diffraction.It was found that the structure solved corresponded to the one reported first in [9].

Characterization
The data set was collected using a Bruker D8 Venture diffractometer with a microfocus sealed tube and a Photon II detector.Monochromated MoKα radiation (λ = 0.71073 Å) was used.Data were collected at 133(2) K and corrected for absorption effects using the multi-scan method.The structure was solved by direct methods using SHELXT [59]) and was refined by full-matrix least squares calculations on F2 (SHELXL2018 [60]) in the graphical user interface Shelxle [61].Powder XRD measurements were performed on a PANalytical Empyrean diffractometer (Malvern PANalytical Empyrean, Almelo, the Netherlands) with a PIXcel 3D detector and CuKα radiation (λ = 0.1542 nm).Microstructural information was extracted by full-profile Rietveld refinement using the GSAS II crystallography software package [62].Infrared spectral analysis was carried out on an FTIR Nicolet 6700 (Thermo Scientific) in KBr pellets.Scanning electron microscopy (Hitachi TM4000; Krefeld, Germany) was used to observe the morphology of the obtained materials.Lifetime measurements and photoluminescence measurements of the complexes were conducted on a Cary Eclipse spectrometer with a xenon lamp as the excitation source.For powder samples, a powder cell with a Cary Eclipse Solid Sample Holder was used, and for suspension measurements, 1 cm fluorescent quartz cuvettes were used.The textural characteristics of the samples were determined by low-temperature nitrogen adsorption.The adsorption and desorption isotherms of nitrogen at −196 • C were determined in the pressure range of p/p 0 = 0.001-1 using "AUTOSORB iQ-MP/AG" (Anton Paar GmbH, Graz, Austria).Before every measurement, the samples were degassed at 250 • C for 16 h.pH measurements were performed using the XS sensor pH 8+ DHS kit BASIC with a micro P electrode.A Q55 Sonicator probe was used for homogenization of the suspensions.The suspensions for all sensing experiments were prepared using the as-prepared MOFs.A stock aqueous suspension with a concentration of 1.0 mg/mL was prepared.The suspension was treated with a Q55 Sonicator probe for several minutes.Next, by dilution, 4 suspensions with concentrations of 0.7, 0.5, 0.3, and 0.1 mg/mL were prepared, followed by sonication and measurement of their luminescence under the same conditions (emission spectra: λex = 320 nm, ex/em slit: 5/2.5 nm, data interval: 1.0 nm, average time: 0.10 s, PMT voltage: 800 V).
For both EuBDC and TbBDC, a 0.5 mg/mL concentration was chosen, demonstrating the best stability and excluding self-quenching effects (Figure S4).

Procedure for pH Measurements of the Suspensions
For both samples, 10 vials with different pH values were prepared.A solution of KCl (0.1 mol/L) was used to keep the ionic strength constant.HCl and KOH (0.1 mol/L) were added to the KCl solution to adjust the pH value in steps of around 1.0.When the desired pH value was reached, a certain volume from the solution was added to the preweighed sample vial so that the concentration of the suspension was adjusted to 0.5 mg/mL.All samples were sonicated and measured under the same conditions (emission spectra: λex = 320 nm, ex/em slit: 5/2.5 nm, data interval: 1.0 nm, average time: 0.10 s, PMT voltage: 800 V).

Procedure for Cation and Anion Sensing Experiments
To explore the behavior of TbBDC and EuBDC in the presence of different cations and anions, 1 mg/mL of a stock aqueous suspension was prepared.Stock solutions of cations and anions with a concentration of 1 × 10 −2 mol/L were used.Cations were nitrate salts, and anions were potassium and sodium salts.Briefly, 1.0 mL of the starting suspension was mixed with 0.8 mL of water and 0.2 mL of the stock solution of cations and anions, so the resulting concentration of the suspensions was 0.5 mg/mL, and the concentration of cations and anions was 1 × 10 −3 mol/L.All samples were then measured with a pH meter (Table S4) to confirm we were in the working pH range of the sensors.

Procedure for Stern-Volmer Data Collections and Data Management
Briefly, suspensions with a starting concentration of 0.5 mg/mL were prepared in two parallel cuvettes, and each was measured five times to determine the standard deviation of the blank sample.Next, to one of them was added the exact volume of the stock solution of the chosen ion, and to the other was added the same volume of water.Each time, both samples were measured three times.Baseline correction was performed, and for each concentration, the average value of the intensity from the parallel measurements was taken (for TbBDC at λ = 547 nm and for EuBDC at λ = 616 nm).Since dilution with water during the experiment in the second cuvette did not lead to a significant decrease in the intensity of the blank sample, we used an average value of all measurements of the blank sample for I 0 .
When working with luminescent sensors, we need to apply the Stern-Volmer equation.The simplest case is to observe the linear dependence of Stern-Volmer data, but it is not an uncommon thing to have nonlinear dependence, suggesting a different quenching mechanism or more than one quenching mechanism taking part.As reported by W. Laws and P. Contino [63], when linear dependence is observed, we may have the dynamic quenching mechanism described by Equation (1): I 0 /I = 1 + K sv [Q] (1) I 0 is the intensity in the absence of a quencher; I is the intensity in the presence of a quencher; K sv is the Stern-Volmer constant corresponding to the dynamic quenching constant K D ; [Q] is the concentration of the quencher.Similarly, Equation (2), with linear dependence, can describe static quenching, where quenching occurs as a result of the formation of a nonfluorescent ground-state complex between the fluorophore and the quencher.
Only here, K S is the association constant.Static quenching removes a fraction of the fluorophores from observation.The complexed fluorophores are nonfluorescent, and the only observed fluorescence is from the uncomplexed fluorophores.The uncomplexed fraction is unperturbed, and hence, the lifetime is τ 0 .Therefore, for static quenching, τ 0 /τ = 1.In contrast, for dynamic quenching, τ 0 /τ follows the same linear dependence as I 0 /I.
When both static quenching and dynamic quenching are combined, we observe both quenching by collisions and quenching by complex formation with the same quencher.The Stern-Volmer equation is a second-order polynomial curve described by Equation (3): The dynamic portion of the observed quenching can be determined by lifetime measurements, i.e., we modify Equation (3) to allow a graphical separation of K S and K D [63][64][65][66].where I is the intercept and S is the slope of the graphical representation of Kapp to the concentration of the quencher.
There is another type of static quenching in which the quencher does not actually form a ground-state complex.Instead, it seems that the apparent static component is due to the quencher being adjacent to the fluorophore at the moment of excitation.These closely spaced fluorophore-quencher pairs are immediately quenched and thus appear to be dark complexes.This quenching is called "sphere of action", within which the probability of quenching is unity.The modified form of the Stern-Volmer equation that describes this situation is Equation ( 5): where V is the volume of the sphere.When the fluorophore and the quencher are this close, there exists a high probability that quenching will occur before these molecules diffuse apart.As the quencher concentration increases, the probability increases that the quencher is within the first solvent shell of the fluorophore at the moment of excitation [63,64].Several studies on sensors with exponential curves have used the modified Equation ( 6): They have calculated the Stern-Volmer constant as a product of constant A and constant k in Equation (7) [67][68][69][70][71].

Figure 2 .
Figure 2. (a) XRD pa erns of the as-prepared LnBDC MOFs compared to the simulated XRD pa ern of the DyBDC-SC and (b) a close look at the 27-32 2θ part confirming the change in the unit cell parameters.

Figure 2 .
Figure 2. (a) XRD patterns of the as-prepared LnBDC MOFs compared to the simulated XRD pattern of the DyBDC-SC and (b) a close look at the 27-32 2θ part confirming the change in the unit cell parameters.

Molecules 2024 ,
29,  x FOR PEER REVIEW 6 of 23 BaSO4 5 wt%).It was clearly observed (Figure4b) that the emissions from TbBDC and EuBDC now were of almost equal intensity.This observation is evidence of the selfquenching effect, significantly influencing the EuBDC emission.Following the results observed, subsequent measurements and experiments on sensor properties were focused mainly on Tb(III) and Eu(III) samples.

Figure 4 .
Figure 4. Comparison of the emissions registered from different types of LnBDC: (a) pure samples in a solid state; (b) 5 wt% LnBDC in BaSO4.

Figure 4 .
Figure 4. Comparison of the emissions registered from different types of LnBDC: (a) pure samples in a solid state; (b) 5 wt% LnBDC in BaSO 4 .

Figure 5 .
Figure 5. Luminescence spectra of freshly prepared and 3-week-aged suspensions of (a) EuBDC and (b) TbBDC.Powder XRD just after synthesis and after 3 weeks' stay in water for (c) EuBDC and (d) TbBDC.

Figure 5 .
Figure 5. Luminescence spectra of freshly prepared and 3-week-aged suspensions of (a) EuBDC and (b) TbBDC.Powder XRD just after synthesis and after 3 weeks' stay in water for (c) EuBDC and (d) TbBDC.

Figure 6 .
Figure 6.Luminescence measurements under the same conditions of 0.5 mg/mL of suspension in different solvents: (a) EuBDC and (b) TbBDC.

Figure 7 .
Figure 7. Luminescence measurements under the same conditions of 0.5 mg/mL of suspension at different pH values: (a) EuBDC and (b) TbBDC.

Figure 6 .
Figure 6.Luminescence measurements under the same conditions of 0.5 mg/mL of suspension in different solvents: (a) EuBDC and (b) TbBDC.

Figure 6 .
Figure 6.Luminescence measurements under the same conditions of 0.5 mg/mL of suspension in different solvents: (a) EuBDC and (b) TbBDC.

Figure 7 .
Figure 7. Luminescence measurements under the same conditions of 0.5 mg/mL of suspension at different pH values: (a) EuBDC and (b) TbBDC.

Figure 7 .
Figure 7. Luminescence measurements under the same conditions of 0.5 mg/mL of suspension at different pH values: (a) EuBDC and (b) TbBDC.

Figure 10 .Figure 11 .
Figure 10.Luminescence of (a) EuBDC (inset: picture of the suspension under a UV lamp with max.254 nm with and without a quencher) and (b) TbBDC at different concentrations of Ag(I) (inset: picture of the suspension under a UV lamp with max.254 nm with and without a quencher).

Figure 10 .
Figure 10.Luminescence of (a) EuBDC (inset: picture of the suspension under a UV lamp with max.254 nm with and without a quencher) and (b) TbBDC at different concentrations of Ag(I) (inset: picture of the suspension under a UV lamp with max.254 nm with and without a quencher).

Figure 10 .Figure 11 .
Figure 10.Luminescence of (a) EuBDC (inset: picture of the suspension under a UV lamp with max.254 nm with and without a quencher) and (b) TbBDC at different concentrations of Ag(I) (inset: picture of the suspension under a UV lamp with max.254 nm with and without a quencher).

Figure 11 .
Figure 11.Stern-Volmer curves for (a) EuBDC and (b) TbBDC (λex = 320 nm).Intensity at 547 nm in the absence of a quencher, divided by the intensity in the presence of a quencher; baseline correction applied.

Figure 13 .
Figure 13.Luminescence spectra of TbBDC in the absence of Ag(I) and at concentrations over 1.8 mM.

Figure 13 .
Figure 13.Luminescence spectra of TbBDC in the absence of Ag(I) and at concentrations over 1.8 mM.

Figure 13 .
Figure 13.Luminescence spectra of TbBDC in the absence of Ag(I) and at concentrations over 1.8 mM.

Figure 14 .
Figure 14.(a) Luminescence at different concentrations of Cr(III) and (b) exponential fit of the data.

Figure 14 .
Figure 14.(a) Luminescence at different concentrations of Cr(III) and (b) exponential fit of the data.

Figure 14 .
Figure 14.(a) Luminescence at different concentrations of Cr(III) and (b) exponential fit of the data.

Figure 16 .
Figure 16.(a) Intensity at 547 nm in the absence of a quencher, divided by the intensity in the presence a of quencher (λex =320 nm); baseline correction applied.(b) Lifetime value in the absence of a quencher, divided by lifetime values in the presence of a quencher.

Figure 16 .
Figure 16.(a) Intensity at 547 nm in the absence of a quencher, divided by the intensity in the presence a of quencher (λex =320 nm); baseline correction applied.(b) Lifetime value in the absence of a quencher, divided by lifetime values in the presence of a quencher.

Figure 17 .
Figure 17.Graphical separation of K S and K D for TbBDC with Fe(III).

Figure 17 .
Figure 17.Graphical separation of KS and KD for TbBDC with Fe(III).

Figure 18 .
Figure 18.Exponential fit of the data for TbBDC with Fe(III).

Figure 18 .
Figure 18.Exponential fit of the data for TbBDC with Fe(III).

Figure 19 .
Figure 19.Polynomic (a) and exponential (b) fit of the data for TbBDC with Cr(VI).

Figure 20 .
Figure 20.Lifetime value in the absence of a quencher, divided by lifetime values in the presence of a quencher.

Figure 19 .
Figure 19.Polynomic (a) and exponential (b) fit of the data for TbBDC with Cr(VI).

Figure 19 .
Figure 19.Polynomic (a) and exponential (b) fit of the data for TbBDC with Cr(VI).

Figure 20 .
Figure 20.Lifetime value in the absence of a quencher, divided by lifetime values in the presence of a quencher.

Figure 20 .
Figure 20.Lifetime value in the absence of a quencher, divided by lifetime values in the presence of a quencher.

Figure 21 .
Figure 21.Normalized absorption of solutions with concentration 1×10 −3 mol/L.In the case of Fe(III) and CrO 4 2−/ Cr 2 O 7 2 − quenching, we have to consider that the luminescence of Ln-MOFs mainly suffers from the "antenna effect", i.e., the ligands efficiently absorb and transfer light to the luminescent central lanthanide ions.As shown in Figure 21, the UV-VIS absorption spectra of Fe(III) and CrO 4 2−/ Cr 2 O 7 2− emerged as strong absorption bands in the range of 200-350 nm for Fe(III) and 260-400 nm for CrO 4 2−/ Cr 2 O 7 2− , while the excitation of LnBDC was at 320 nm.These facts imply that Fe(III) and CrO 4 2−/ Cr 2 O 7 2 could drastically absorb the energy of the excitation, reducing